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NOMENCLATURE

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the forces that hold two or more atoms together to form a compound. ... Cupric chloride. Binary Ionic Compounds (Type II): Naming Compounds (continued) ... – PowerPoint PPT presentation

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Title: NOMENCLATURE


1
NOMENCLATURE
  • Chapter 5

2
Charges on Common Ions
-4
-3
-2
-1
1
2
3
3
Table 5.1 Common Simple Cations and Anions
4
Chemical Bonds
  • - the forces that hold two or more atoms together
    to form a compound.
  • - the two types of chemical bonds are
  • 1. Ionic bonds.
  • NaCl KI
  • 2. Covalent bonds.
  • H2O CH4

metal nonmetal
two nonmetals
5
Chemical Bonds(continued)
  • Ionic Bonding Force of attraction between
    oppositely charged ions.
  • - Chemical compounds must have a net charge of
    zero.
  • 1. Both cations and anions must be present.
  • 2. The number of cations and anions must be
    such that the net charge is zero.

6
Writing Formulas for Ionic Compounds
Charge must equal zero for each compound.
1 1- 0 2 2- 0 6 6- 0
7
COMPOUNDS FORMED FROM IONS
  • CATION ANION ---gt
  • COMPOUND
  • Na Cl- --gt NaCl
  • A neutral compound requires equal number of ()
    and (-) charges.

8
Chemical Bonds(continued)
  • Covalent bonding results from atoms sharing
    electrons.
  • Molecule a collection of covalently-bonded
    atoms.
  • H2O C12H22O11

9
Common Names
  • sugar of lead
  • blue vitriol
  • quicklime
  • Epsom salts
  • milk of magnesia
  • gypsum
  • laughing gas

lead(II) acetate copper(II) sulfate calcium
oxide magnesium sulfate magnesium
hydroxide calcium sulfate dinitrogen monoxide
10
Common Names - Exceptions
  • H2O water, steam, ice
  • NH3 ammonia
  • CH4 methane
  • NaCl table salt
  • C12H22O11 table sugar

11
Types of Cations
  • Type I Cations
  • only one charge
  • Group I ions
  • Group II ions
  • Aluminum
  • Cadmium
  • Silver
  • Zinc
  • Memorize Table 5.1, page 129
  • Type II Cations
  • more than one charge
  • transition elements
  • elements under the stairstep
  • Memorize Table 5.2, page 133

12
Metal Cations
  • Type I
  • Metals that can only have one possible charge
  • Determine charge by position on the Periodic
    Table
  • Type II
  • Metals that can have more than one possible
    charge
  • Determine metal cations charge from the charge
    on anion

13
Naming Compounds
Binary Ionic Compounds
  • 1. Cation first, then anion
  • 2. Monatomic cation name of the element
  • Ca2 calcium ion
  • 3. Monatomic anion root -ide
  • Cl? chloride
  • CaCl2 calcium chloride

14
Naming Compounds(continued)
Binary Ionic Compounds (Type II)
  • - metal forms more than one cation
  • - use Roman numeral in name
  • CuCl2 Cu2 is cation
  • CuCl2 Copper (II) chloride
  • Cupric chloride

15
Naming Compounds(continued)
Binary compounds (Type III)
  • - Compounds between two nonmetals
  • - First element in the formula is named first.
  • - Second element is named as if it were an anion.
  • - Use prefixes (Table 5.3 on page 137).
  • - Never use mono- for the first element.
  • P2O5 diphosphorus pentoxide

16
Prefixes
  • Drop last a in the prefix if the name begins
    with vowel

17
Figure 5.1 A flow chart for naming binary
compounds.
18
Common Nomenclature Mistakes
  • Compounds
  • SO3 --Sulfur trioxide
  • NO2 -- Nitrogen dioxide
  • NO3 -- Nitrogen trioxide
  • NH3 -- Ammonia
  • Polyatomic ions
  • SO32- -- Sulfite ion
  • NO21- -- Nitrite ion
  • NO31- -- Nitrate ion
  • NH41 --Ammonium ion

19
MOLECULAR FORMULAS
  • Formula for glycine is C2H5NO2
  • In one molecule there are
  • 2 C atoms
  • 5 H atoms
  • 1 N atom
  • 2 O atoms

20
Molecular Modeling
Drawing of glycine
Ball stick
Space-filling
21
POLYATOMIC IONS
  • Groups of atoms with a charge.
  • MEMORIZE the names and formulas in Table 5.4,
    page 142.

22
Table 5.4 Names of Common Polyatomic Ions
23
Patterns for Polyatomic Ions
  • -ate ion
  • chlorate ClO3-
  • -ate ion plus 1 O ? same charge, per- prefix
  • perchlorate ClO4-
  • -ate ion minus 1 O ? same charge, -ite suffix
  • chlorite ClO2-
  • -ate ion minus 2 O ? same charge, hypo- prefix,
    -ite suffix
  • hypochlorite ClO-

24
Some Common Polyatomic Ions
  • NH4 ammonium ion One of the few common
    polyatomic cations

25
Some Common Polyatomic Ions
  • CO32- carbonate ion
  • HCO3- bicarbonate ion
  • - hydrogen carbonate ion

26
Some Common Polyatomic Ions
  • SO42- sulfate ion
  • SO32- sulfite ion

27
Some Common Polyatomic Ions
  • NO3- nitrate ion
  • NO2- nitrite ion

28
Figure 5.2 Overall strategy for naming chemical
compounds
29
NOMENCLATURE OF COMPOUNDS
Binary -- 2 elements
Ternary -- (3 elements) - Ionic
(metal ion polyatomic ion)
Ca3(PO4)2 -- calcium phosphate FeSO4 -- iron
(II) sulfate -- ferrous sulfate
Type I - Ionic (Type I metal
nonmetal) Group I, II, Al3, Ag1, Cd2,
Zn2 NaCl -- Sodium Chloride
Type II - Ionic (Type II metal nonmetal) All
other metals Fe2S3 -- iron (III) sulfide
-- ferric sulfide
Type III - covalent (2 nonmetals) CO2 -- carbon
dioxide
30
Binary Acids
  • made up of two elements -- hydrogen and a
    nonmetal
  • named by using
  • prefix hydro root of nonmetal ic acid
  • HCl -- hydrochloric acid
  • H2Se -- hydroselenic acid

31
Table 5.5 Names of Acids that Do Not Contain
Oxygen
32
Ternary Acids (oxyacids)
  • contain three elements -- hydrogen, nonmetal,
    and oxygen.
  • most oxygen per root of nonmetal ic
    acid
  • less oxygen root of nonmetal ic acid
  • less oxygen root of nonmetal ous acid
  • least oxygen hypo root of nonmetal ous
    acid

33
Ternary Acids(continued)
  • HBrO4 perbromic acid
  • HBrO3 bromic acid
  • HBrO2 bromous acid
  • HBrO hypobromous acid
  • H3PO4 phosphoric acid
  • H3PO3 phosphorous acid
  • H3PO2 hypophosphorus acid

34
Figure 5.3 A flow chart for naming acids
35
Salt Nomenclature (continued)
  • Ternary salts ( metal and polyatomic ion)
  • name of positive ion root of nonmetal ate or
    ite
  • If the salt comes from an ic acid, change ic to
    ate.
  • H2CO3 carbonic acid Na2CO3 sodium carbonate
  • H3PO4 phosphoric acid K3PO4 potassium
    phosphate
  • If the salt comes from an ous acid, change ous to
    ite.
  • H2SO3 sulfurous acid Li2SO3 lithium sulfite
  • HClO hypochlorous acid NaClO sodium
    hypochlorite

36
Chemical Nomenclature
  • Name each of the following
  • CuCl
  • HgO
  • Fe2O3
  • MnO2
  • PbCl2
  • CrCl3

copper(I) chloride cuprous
chloride mercury(II) oxide mercuric
oxide iron(III) oxide ferric
oxide manganese(IV) oxide manganic
oxide lead(II) chloride plumbous
chloride chromium(III) chloride chromic
chloride
37
Chemical Nomenclature
  • Name each of the following
  • P4O10
  • N2O5
  • Li2O2
  • Ti(NO3)4
  • SO3
  • SF6
  • O2F2

tetraphosphorus decoxide dinitrogen
pentoxide lithium peroxide titanium(IV)
nitrate sulfur trioxide sulfur hexafluoride dioxyg
en difluoride
38
Writing the Formulas from the Names
  • For Type III compounds, use the prefixes to
    determine the subscripts
  • For Type I, Type II, polyatomic Compounds and
    Acids
  • Determine the ions present
  • Determine the charges on the cation and anion
  • Balance the charges to get the subscripts

39
Determining the Charge on a Cation Au2S3
  • Determine the charge on the anion
  • Au2S3 - the anion is S, since it is in Group 6A,
    its charge is -2
  • Determine the total negative charge
  • since there are 3 S in the formula, the total
    negative charge is -6
  • Determine the total positive charge
  • since the total negative charge is -6, the total
    positive charge is 6
  • Divide by the number of cations
  • since there are 2 Au in the formula the total
    positive charge is 6, each Au has a 3 charge
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